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2b. Ch 4 Barium hydroxide sulfuric acid titration

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Barium Hydroxide
Sulfuric Acid Reaction
Please view the titration movie
before viewing this presentation
Problem
Aqueous barium hydroxide and
sulfuric acid solutions are mixed
together.
a. What products are formed?
b. What are the molecular, total ionic and net
ionic reactions?
Ba(OH)2(aq)
Ba2+(aq)
OH-(aq)
H2SO4(aq)
OH-(aq)
H2O(L)
BaSO4(s)
H+(aq)
H+(aq)
SO42-(aq)
Equations:
Molecular Equation:
H2SO4(aq)

2 H2O(L)
+
BaSO4(s)
Ba2+(aq) + 2 OH- (aq) + 2 H+(aq) + SO42-(aq)

2 H2O(L)
+
BaSO4(s)

2 H2O(L)
+
BaSO4(s)
Ba(OH)2(aq)
+
Total Ionic Equation:
Net Ionic Equation: NO Spectator ions!
Ba2+(aq) + 2 OH- (aq) + 2 H+(aq) + SO42-(aq)
Why did the light bulb go out?
No Ions Present!
At the titrations equivalence, all ions had
combined to form BaSO4(s) and H2O(L)
Adding more H2SO4:
Why did the light bulb relight?
Ions are again present!
No Ba(OH)2 left.
The ions from excess H2SO4 had nothing to
react with and thus increased the ion
content of the solution
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